Zumdahl Chemistry 7th ed. Ch. 1&2 Flashcards
These cards are based on the following text: "Chemistry (Seventh Edition) by Zumdahl & Zumdahl"
Some things from Chapters 1 & 2 have been left out because they cannot effectively be studied through flashcards.
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Note: Taken from a set already made and tailored for CH102 at the University of Guam
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| 454704914 | What is the formula for % error? | IEv-TvI/Tv x 100 Where Ev = experimental value and Tv = True value |  | 1 |
| 454704915 | What is an alternate formula for temperature conversions from Fahrenheit to Celsius? | Temp F +40 / Temp C + 40 = 9*F/5*C |  | 2 |
| 454704916 | What is the denisty formula? | d = m / v |  | 3 |
| 454704917 | What is the useful conversion factor that allows you to convert from liters to meters or vice-versa? | 1 mL = 1 cm³ | 4 | |
| 454704918 | Technically speaking, what is a solution? | A homogenous mixture | 5 | |
| 454704919 | What does "homogenous" mean? | Having visually indistinguishable parts | 6 | |
| 454704920 | What does "heterogeneous" mean? | Having visibly distinguishable parts | 7 | |
| 454704921 | What is mass? | Simply: the quantity of matter in an object Complicatedly: A measure of the resistance of an object to a change in its state of motion. Measured by the force necessary to give an object a certain accerlation. (Extra info: On earth we use the force that gravity exerts on an object to measure its mass, this force is called an object's weight) | 8 | |
| 454704922 | SI unit for Mass? | kilogram (kg) | 9 | |
| 454704923 | SI unit for Length? | meter (m) | 10 | |
| 454704924 | SI unit for Time? | second (s) | 11 | |
| 454704925 | SI unit for Temperature? | kelvin (K) | 12 | |
| 454704926 | SI unit for Amount of substance? | mole (mol) | 13 | |
| 454704927 | What is the SI system? | le Systéme International (International System). An Internationally agreed upon (1960) system of units derived from the metric system. | 14 | |
| 454704928 | T/F: Measurements are always certain. | False, there is always some degree of uncertainity (this is where significant figures comes into play) | 15 | |
| 454704929 | What is accuracy? | The agreement of a particular value with the true value. | 16 | |
| 454704930 | What is precision? | The degree of agreement among several measurments of the same quantity. | 17 | |
| 454704931 | What are the two types of error? Describe each. | Random Error: (indeterminate error) a measurmeant has an equal probability of being high or low. Systematic Error: (determinate error) either always high or always low; the error occurs in the same direction each time. | 18 | |
| 454704932 | What is a pure substance? | A substance with constant composition. | 19 | |
| 454704933 | What is a mixture? | A mixture of pure substances with variable composition. | 20 | |
| 454704934 | What is a physical change? | Change in the form of a substance, not its chemical composition. (Example: when water freezes/boils it changes its state but is still composed of H2O molecules) | 21 | |
| 454704935 | Can a physical change separate a mixture into pure compounds? | Yes. What it can't do is break compounds into elements. | 22 | |
| 454704936 | 1 in = ? cm | 1 in = 2.54 cm | 23 | |
| 454704937 | 1 mi = ? ft | 1 mi = 5280 ft | 24 | |
| 454704938 | 1 lb = ? oz | 1 lb = 16 oz | 25 | |
| 454704939 | 1 lb = ? g | 1 lb = 453.6 g | 26 | |
| 454704940 | 1 L = ? qt | 1.06 qt | 27 | |
| 454704941 | 1 gal = ? qt | 1 gal = 4 qt | 28 | |
| 454704942 | What is a compound? | A substance composed of 2 or more elements with constant composition. | 29 | |
| 454704943 | Are elements decomposed into simpler substances by chemical or physical means? | Neither. Elements cannot be decomposed into simpler substances by chemical or physical means. | 30 | |
| 454704944 | What is temperature? | A measure of the random motion of atoms/molecules on a macroscopic level, a measure of the heat intensity. | 31 | |
| 454704945 | What are three methods for separating components of mixture? | - Distillation. - Filtration - Chromatography | 32 | |
| 454704946 | Describe Distillation. | Depends on volatility (how readily subst. becomes gas). Simple distillation: Heat subst., vaporizes, vapor passes through cooled tube (condenser), vapor condenses back to liquid. | 33 | |
| 454704947 | Describe Filtration. | Used when mixture consits of solid & liquid. Mixture poured onto mesh, passes the liquid and leaves the solid behind. | 34 | |
| 454704948 | Describe Chromatography | Uses two phases (states) of matter: mobile & stationary. Paper Chromat: Drop of mixt. placed on paper, dipped into liquid (mobile phase), liqd. travels up paper. | 35 | |
| 454704949 | What is mass number? | # of proton and # of neutron in atom. This is not on the Periodic Table This is represented by the letter A. | 36 | |
| 454704950 | What is atomic number? | # of protons in atom. This is represented by the letter Z. This denotes position of element (based on number of protons) on periodic table. | 37 | |
| 454704951 | How are mass number and atomic number depicted with the element symbol? | Recall: Mass # (A) = # of proton + # of neutron Atomic # (Z) = # of proton |  | 38 |
| 454704952 | Sb | Antimony (Original name: Stibium) | 39 | |
| 454704953 | Cu | Copper (Original name: Cuprum) | 40 | |
| 454704954 | Fe | Iron (Original name: Ferrum) | 41 | |
| 454704955 | Pb | Lead (Original name: Plumbum) | 42 | |
| 454704956 | Hg | Mercury (Original name: Hydrargyrum) | 43 | |
| 454704957 | K | Potassium (Original name: Kalium) | 44 | |
| 454704958 | Ag | Silver (Original name: Argentum) | 45 | |
| 454704959 | Na | Sodium (Original name: Natrium) | 46 | |
| 454704960 | Sn | Tin (Original name: Stannum) | 47 | |
| 454704961 | W | Tungsten (Original name: Wolfram) | 48 | |
| 454704962 | What is Avogadro's Hypothesis? | At the same temperature and pressure, equal volumes of different gases contain the same number of particles. | 49 | |
| 454704963 | J.J. Thomson is important for...? | e/m = -1.76 x 10^8C/g Cathode-ray tubes: Ray produced at negative electrode, it was repelled by negative pole of electric fieled -> JJ thought ray was stream of negatively charged particles (now called electrons). Plum Pudding Model - electrons like rasin dispersed in pudding (incorrect) Charge-to-mass ratio of electron: e represents charge on electron in coulombs (C) m represents electron mass (g) |  | 50 |
| 454704964 | Robert Millikan is important for...? | Oil drop experiments -> determined magnitude of electron charge. This value + charge-to-mass (from JJ T.) = mass of the electron (9.11 x 10⁻³¹ kg) | 51 | |
| 454704965 | Ernest Rutherford is important for...? | Tested JJ's PlumPudding model. Directed α particles towards thin metal foil. (If JJ right, particles should pass through foil w/ minor deflection) most did go straight BUT many were deflected @ large angles & some totally reflected. Deflections could only be caused by concentrated + charged center (containing most mass) | 52 | |
| 454704966 | If atoms are composed of the same components, why do different atoms have different chemical properties? | Answer lies in the number and arrangement of electrons. More electrons allows for more "intermingling" for atoms to combine to form molecules. | 53 | |
| 454704967 | What is an isotope? | An atom with the same number of protons but different number of neutrons | 54 | |
| 454704968 | A positive ion is...? | A cation | 55 | |
| 454704969 | A negative ion is...? | An anion | 56 | |
| 454704970 | What is an ion | An atom or group of atoms that has a net positive or negative charge. | 57 | |
| 454704971 | What is ionic bonding? | Force of attraction between oppositely charged ions. | 58 | |
| 454704972 | Characteristics of metals? | Physical Properties: efficient conduction of heat & electricity, malleability (hammer into thin sheets), ductility (pull into wires), lustrous appearance. Chemically: tend to lose electrons (form + ions) |  | 59 |
| 454704973 | Characteristics of nonmetals? | Chemically: gain electrons to form - ions, often bond to each other (forming covalent bonds), Found in: Upper-right corner of table (except H) | 60 | |
| 454704974 | How is the Periodic Table divided? | Rows: #'s used to identify "periods" Columns: Called groups or families. Have similar chemical properties. | 61 | |
| 454704975 | Where are the alkali metals? Briefly describe them. | Group 1A. Very active elements that readily form ions with a 1+ charge, when they react with nonmetals. |  | 62 |
| 454704976 | Where are the halogens? Briefly describe them. | Group 7A. All form diatomic molecules. |  | 63 |
| 454704977 | Where are the noble gases? Briefly describe them. | Group 8A. They all exist (under normal conditions) as monatomic (single-atom) gases. Have little chemical reactivity. |  | 64 |
| 454704978 | Where are the alkaline earth metals? Briefly describe them. | Group 2A. They all form ions with a 2+ charge, when they react with nonmetals. |  | 65 |
| 454704979 | 1 m = ? yd | 1 m = 1.094 yd | 66 | |
| 454704980 | 1 kg = ? lb | 1 kg = 2.205 lb | 67 | |
| 454704981 | 1 ft³ = ? L | 1 ft³ = 28.32 L | 68 | |
| 454704982 | Where are the Lanthanides? | Element 58 - 71 (top row at the bottom) |  | 69 |
| 454704983 | Where are the transition metals? |  | 70 | |
| 454704984 | Where are the Actinides? | Elements 90 - 103 (bottom of bottom) |  | 71 |
| 454704985 | Briefly describe Dalton's atomic theory | - all elements are composed of atoms - all atoms of a given element are identical - chemical compounds are formed when atoms combine - atoms are not changed in chemical reactions but the way they are bound together changes | 72 | |
| 454704986 | Define: Law of Conservation of Mass | Mass is neither created nor destroyed. | 73 | |
| 454704987 | Define: Law of Definite Proportion | A given compound always contains exactly the same proportion of elements by mass. | 74 | |
| 454704988 | Define: Law of Multiple Proportions | When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers. | 75 | |
| 454704989 | At room temperature which elements are solid? | All metals [except Hg(l) ] + some others | 76 | |
| 454704990 | At room temperature which elements are liquid? | Hg(l) and Br₂(l) | 77 | |
| 454704991 | At room temperature which elements are gas? | All the noble gases and H₂, N₂, O₂, F₂, Cl₂ | 78 | |
| 454704992 | Which molecules are diatomic? | H₂(g), N₂(g), O₂(g), F₂(g), Cl₂(g), Br₂(l), I₂(s), At₂(s) Notice all of the halogens are diatomic. | 79 |